What Is The Chemical Makeup Of Lithium

Chemistry of Lithium (Z=3)

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Lithium is a rare chemical element found primarily in molten rock and saltwater in very small amounts. It is understood to be not-vital in human biological processes, although it is used in many drug treatments due to its positive effects on the human brain. Considering of its reactive properties, humans have utilized lithium in batteries, nuclear fusion reactions, and thermonuclear weapons.

Introduction

Lithium was kickoff identified as a component of of the mineral petalite and was discovered in 1817 by Johan August Arfwedson, but not isolated until some time later on by West.T. Brande and Sir Humphry Davy. In its mineral forms it accounts for only 0.0007% of the earth's crust. Information technology compounds are used in certain kinds of drinking glass and porcelain products. More recently lithium has become important in dry-prison cell batteries and nuclear reactors. Some compounds of lithium have been used to care for manic depressives.

Lithium is an element of group i with the atomic number = 3 and an atomic mass of 6.941 g/mol. This means that lithium has iii protons, 3 electrons and 4 neutrons (6.941 - three = ~4). Beingness an brine metallic, lithium is a soft, combustible, and highly reactive metal that tends to form hydroxides. Information technology also has a pretty depression density and under standard conditions, it is the least dense solid element.

Properties

Lithium is the lightest of all metals and is named from the Greek piece of work for stone (lithos). It is the outset member of the Brine Metallic family. It is less dense than water (with which information technology reacts) and forms a blackness oxide in contact with air.

Table 1. Properties of lithium.
Atomic Number	iii
Diminutive Mass	6.941 g/mol
Atomic Radius	152 pm
Density	0.534 grand/cmⁱⁱⁱ
Colour	calorie-free silver
Melting point	453.69 Grand
Boiling point	1615 Thou
Oestrus of fusion	3.00 kJ/mol
Heat of vaporization	147.1 kJ/mol
Specific heat capacity	24.860 kJ/mol
First ionization energy	520.two kJ/mol
Oxidation states	+1, -i
Electronegativity	0.98
Crystal structure	trunk-centered cubic
Magnetism	paramagnetic
2 stable isotopes	^sixLi (seven.5%) and ⁷Li (92.5%)

Periodic Trends of Lithium

Being on the upper left side of the Periodic Table, lithium has a fairly low electronegativity and electron affinity every bit compared to the rest of the elements. Also, lithium has high metal character and subsequently lower nonmetallic character when compared with the other elements. Lithium has a higher atomic radius than most of the elements on the Periodic Table. In compounds lithium (like all the alkali metals) has a +1 charge. In its pure form it is soft and argent white and has a relatively low melting point (181oC).

Reactivity

Lithium is part of the Group 1 Alkali Metals , which are highly reactive and are never institute in their pure course in nature. This is due to their electron configuration, in that they have a single valence electron (Effigy 1) which is very easily given upward in order to create bonds and course compounds.

_↑ ↓ _ _↑__

1sⁱⁱ 2s¹

Reactions with H2o

When placed in contact with water, pure lithium reacts to course lithium hydroxide and hydrogen gas.

\[ 2Li (due south) + 2H_2O (fifty) \rightarrow 2LiOH (aq) + H_2 (g)\]

Out of all the group 1 metals, lithium reacts the least violently, slowly releasing the hydrogen gas which may create a vivid orange flame just if a substantial amount of lithium is used. This occurs because lithium has the highest activation energy of its group - that is, information technology takes more than energy to remove lithium's one valence electron than with other grouping 1 elements, because lithium's electron is closer to its nucleus. Atoms with higher activation energies will react slower, although lithium will release more than total heat through the entire process.

Reactions with Air

Pure lithium will form lithium hydroxide due to moisture in the air, also as lithium nitride (\(Li_3N\)) from \(N_2\) gas, and lithium carbonate \((Li_2CO_3\)) from carbon dioxide. These compounds requite the usually the silver-white metal a blackness tarnish. Additionally, it will combust with oxygen as a blood-red flame to class lithium oxide.

\[ 4Li (south) + O_2 (g) \rightarrow 2Li_2O \]

Applications

In its mineral forms it accounts for but 0.0007% of the globe's chaff. It compounds are used in certain kinds of glass and porcelain products. More recently lithium has become important in dry-cell batteries and nuclear reactors. Some compounds of lithium have been used to treat manic depressives.

Batteries

Lithium is able to be used in the function of a Lithium battery in which the Lithium metal serves every bit the anode. Lithium ions serve in lithium ion batteries (chargeable) in which the lithium ions move from the negative to positive electrode when discharging, and vice versa when charging.

Heat Transfer

Lithium has the highest specific rut chapters of the solids, Lithium tends to be used as a cooler for heat transfer techniques and applications.

Sources and Extraction

Lithium is most usually institute combined with aluminum, silicon, and oxygen to class the minerals known as spodumene (LiAl(SiO_iii)_two) or petalite/castorite (LiAlSi₄O_x). These have been found on each of the half-dozen inhabited continents, but they are mined primarily in Western Commonwealth of australia, Communist china, and Chile. Mineral sources of lithium are condign less essential, as methods have now been developed to make use of the lithium salts institute in saltwater.

Extraction from minerals

The mineral forms of lithium are heated to a high plenty temperature (1200 Grand - 1300 Thousand) in club to crumble them and thus allow for subsequent reactions to more easily accept place. Afterward this process, 1 of iii methods can be applied.

The use of sulfuric acid and sodium carbonate to allow the iron and aluminum to precipitate from the ore - from there, more sodium carbonate is applied to the remaining material allow the lithium to precipitate out, forming lithium carbonate. This is treated with muriatic acid to course lithium chloride.
The use of limestone to calcinate the ore, and then leaching with water, forming lithium hydroxide. Once more, this is treated with hydrochloric acrid to class lithium chloride.
The utilise of sulfuric acid, and and then leaching with water, forming lithium sulfate monohydrate. This is treated with sodium carbonate to form lithium carbonate, and and then muriatic acid to course lithium chloride.

The lithium chloride obtained from any of the three methods undergoes an oxidation-reduction reaction in an electrolytic cell, to split the chloride ions from the lithium ions. The chloride ions are oxidized, and the lithium ions are reduced.

\[2Cl^- - 2e^- \rightarrow Cl_2 \;\; \text{(oxidation)}\]

\[Li^+ + e^- \rightarrow Li \;\; \text{(reduction)}\]

Extraction from Saltwater

Saltwater naturally contains lithium chloride, which must be extracted in the form of lithium carbonate, then it is re-treated, separated into its ions, and reduced in the same electrolytic process as in extraction from lithium ores. Only 3 saltwater lakes in the earth are currently used for lithium extraction, in Nevada, Chile, and Argentina.

Saltwater is channeled into shallow ponds and over a period of a year or more, water evaporates out to leave behind diverse salts. Lime is used to remove the magnesium salt, so that the remaining solution contains a adequately concentrated amount of lithium chloride. The solution is then treated with sodium carbonate in order for usable lithium carbonate to precipitate out.

References

Kipouros, Georges J and Sadoway, Donald R. "Toward New Technologies for the Production of Lithium." Journal of Metals. The Minerals, Metals, & Materials Lodge. Volume 50, No. 5 May 1998: 24-32.
Shin, Y. J. ; Kim, I. S. ; Oh, S. C. ; Park, C. K. and Lee, C. S. "Lithium Recovery from Radioactive Molten Table salt Wastes by Electrolysis." Journal of Radioanalytical and Nuclear Chemistry. Akadémiai Kiadó and Springer Science+Business concern Media B.V. Volume 243, No. iii March 2000: 639-643.
Tahil, William. "The Trouble with Lithium - Implications of Future PHEV Production for Lithium Demand." Peak International Research. January 2007.

Problems

With which group of elements will lithium course compounds the almost easily with?
What is the electron configuration of Li⁺?
What are some common uses of lithium?
For a lithium-ion battery containing LiCoO_ii, should the compound be placed in the anode or cathode?
Given that ⁷Li is vii.0160 amu and ⁶Li is 6.0151 amu, and their percent abundance is 92.58% and 7.42% respectively, what is the atomic mass of lithium?

Solutions

Group 17 Halogens (lithium forms strongly inic bonds with them, equally halogens are highly electronegative and lithium has a costless electron)
1s²
Lithium-ion batteries, dispensable lithium batteries, pyrotechnics, cosmos of potent metal alloys, etc.
Anode - lithium is oxidized (LiCoO_two → Li⁺ + CoO₂)
6.942 g/mol

Contributors and Attributions

Katherine Szelong (UCD), Kevin Fan

Source: https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Descriptive_Chemistry/Elements_Organized_by_Block/1_s-Block_Elements/Group__1%3A_The_Alkali_Metals/Z003_Chemistry_of_Lithium_(Z3)

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